CHEM 112 Lecture Notes - Lecture 2: Standard Electrode Potential, Standard Hydrogen Electrode, Faraday Constant
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Any electrode at which the reduction half reaction shows a lesser tendency to occur than the reduction of h+ to h2 , has a standard electrode potential, e o , which is negative. The reaction zn(s) + cu2+(aq) zn2+(aq) + cu(s) in an electrochemical cell. E o cell = e o (right) - e o (left) = e o (cathode) - e o (anode) = e o (reduction half-cell) e o (oxidation half-cell) = e o (cu2+/cu) - e o (zn2+/zn) When an oxidation-reduction reaction occurs in a voltaic cell, the cell is doing electrical work, the work of moving electrical charges. And if the reactants and products of the oxidation-reduction reaction are in their standard states, we have: The value of dgo for this reaction is specific to the stoichiometric coefficients used in the overall reaction (e. g. one h2 to one cu2+)
